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Chapter 12: Atoms & the Periodic Table

Chapter 12: Atoms & the Periodic Table. Atoms Elements Atomic Structure The Periodic Table Spectroscope Identification Quantum Hypothesis Electron Waves Shell Model. Matter. The stuff things are made of. Has Mass and takes up space. (Air, water, rocks, metals etc..).

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Chapter 12: Atoms & the Periodic Table

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  1. Chapter 12: Atoms & the Periodic Table • Atoms • Elements • Atomic Structure • The Periodic Table • Spectroscope Identification • Quantum Hypothesis • Electron Waves • Shell Model

  2. Matter • The stuff things are made of. • Has Mass and takes up space. • (Air, water, rocks, metals etc..) • The amount of stuff (in g’s) • (Bowling Ball > Balloon) Weight on earth. Pull of Gravity on matter.

  3. Atoms & Elements • Matter made up of only one type of atom.

  4. Atomic Symbols Nitrogen Hydrogen Bromine Aluminum Nickel Each element is assigned a unique symbol 1-2 letters; 1st is capitalized

  5. Atomic Symbols Sodium (Natrium) Potassium (Kalium) Silver (Argentum) Lead (Plumbum) Iron (Ferrum) Gold (Aurum) The original name is often of Latin or Greek origin

  6. Atomic Symbols Carbon Calcium Cobalt Copper (Cu) Chlorine Chromium Elements with same starting letter, get second letter added to the symbol

  7. A model of matter • Atom - The smallest unit of an element that is still thatelement. ie. Aluminum (Al) • Molecule -The smallest unit of a pure substance that is still that substance. • May contain > 1 atom or element. ie. Water (H2O)

  8. Structure of the atom Nucleus Small, dense, + charge in the center of an atom. + contains protons + + + + + & neutrons

  9. Structure of the atom • Nucleus (+) Electrons - charged particles that surround the nucleus. Electrons moved around nucleus in orbitals.

  10. Structure of the atom • The nucleus is a small part of an atom. If the nucleus was the size of a marble, the atom would fill a football stadium. The nucleus would weigh over 10,000 tons.

  11. Atomic Symbols A = Atomic mass (amu) = # protons+# neutrons - - X A - - Z + + Z = Atomic number = # protons = # electrons - + + + + -

  12. Atomic Symbols A = Atomic mass = # p+# n C = Charge = + or - values X A C Z # Z = Atomic # # p = # e # = Number of atoms in a formula.

  13. Atomic Symbols A = Atomic mass = # protons+# neutrons 6 6 - - X 12 - - 6 + + Z = Atomic number = # protons = # electrons - + + + + -

  14. Atomic Symbols A = Atomic mass = # protons+# neutrons - - C 12 - - 6 + + Z = Atomic number = # protons = # electrons - + + + + -

  15. Atomic Symbols A = Atomic mass = p + n = 23 C = Charge = +1 11 12 23 1+ Na 11 # = 1 atom in formula. Z = Atomic # = p = 11 Sodium

  16. Why is the atomic weight on the tables not a whole #? 47 Atomic number Name of the element Elemental Symbol Silver Ag 107.87 Atomic mass (weight) Atomic weight = The average, relative mass of an atom in an element.

  17. Isotopes of Hydrogen • Isotopes = Atoms of the same element but having different masses. 1 1 2 1 3 1 H H H - - - + + + Protium 99.99% Tritium Trace % Deuterium 0.01%

  18. Isotopes of Hydrogen Isotopes = Atoms of the same element but having different masses. 1 1 2 1 3 1 H H H - - - + + + Average Atomic weight of Hydrogen = 1.00794amu

  19. Isotopes of Carbon 12 13 14 C C C 6 6 6 - - - - - - - - + + + - + + + + + + + + + - - + + + + + + - - - - - - - 98.89% 1.11% Trace % Average Atomic weight of C= 12.011amu

  20. 14 3 1 C H 6 - - - - + + + + + - + + - - Radioactive Isotopes H-3 C-14 Nucleus is unstable So falls apart (decays) Giving radioactive particles

  21. 37 Cl 17 35 Cl 17 Average Atomic Mass 75.8% 24.2% 35 (75.8) 100 + 37 (24.2) 100 = 35.45 amu

  22. The atomic symbol & isotopes Complete the table: 1 3 2 31 15 P 15 16 15 138 56 Ba 56 82 56 238 92 U 92 46 92

  23. Atomic Structure Complete the table: 2 1 5 3 6 4 Be 4 9 4 5 4 Cl 17 37 17 20 17 Si 14 28 14 14 14

  24. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Modern periodic table • Mendeleev, 1871 • “Properties of the elements • vary in a periodic manner.” I A II A III A IV A V A VI A VIIA VIIIA 1 2 3 4 5 6 7 • The periodic table • helps us understand • behavior, • reactions • properties • of the elements. III B IVB V B VIB VIIB VIII B IB IIB Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

  25. A row or period Periods are assigned numbers H He 1 2 3 4 5 6 7 Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

  26. Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Common group names Noble gases Alkali Metals Halogens Alkaline Earth Metals VIIIA I A Chalcogens H He II A III A IV A V A VI A VIIA Transition Metals Li Be B C N O F Ne Na Mg Al Si P S Cl Ar III B IVB V B VIB VIIB VIII B IB IIB K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Lanthanides Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Actinides

  27. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Why do we have thoserows on the bottom? This arrangement takes too much space and is hard to read.

  28. Names & Symbols Know the names & symbols H He 1 2 3 4 5 6 7 Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

  29. Metals Lustrous, malleable and ductile. Conductors (heat & electricity) Solids at room temp (except Hg) Lose electrons to non-metals. H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar Co K Ca Sc Ti V Cr Mn Fe Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe I Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

  30. B Si As Te At Non-metals H He Li Be C N O F Ne Na Mg Al P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Kr Gas, liquid, solid (dull, brittle) Poor conductors = Insulators Many are diatomic molecules. Gain e’s from metals Share e’s with other non-metals Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb I Xe Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po Rn Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

  31. Metaloids H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe I Intermediate properties Semi conductors Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 3 - 11

  32. Metals Non-metals Metaloids He H C N O F Ne B Li Be P S Cl Ar Si Na Mg Al Se Br Kr Co Ge As K Ca Sc Ti V Cr Mn Fe Ni Cu Zn Ga I Xe Sb Te Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Rn At Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

  33. Solid Liquid Gas Elemental states atroom temperature H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Ls Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 3 - 13 • Chemeketa Community College: Chemistry for Allied Health

  34. Models of Matter

  35. Models of Matter

  36. Models of Matter

  37. Rutherford’s Gold-Foil Experiment • 99% of + particles aimed at gold went straight through. • A few were deflected. • A few bounced back Conclusion: • Atoms are mostly empty space. • Atoms have a small, dense nucleus with + charge.

  38. Models of Matter

  39. Electronic arrangement A new layer is added for each row or period in the table.

  40. 24 12 Mg Electron arrangement Electrons fill layers around nucleus Low  High 32 18 8 2 Shells = Energy levels

  41. 1 1 4 2 H He 9 4 Be 7 3 Li IA IIA 2, 1 2, 2

  42. 1 1 H 11 5 9 4 B Be 7 3 Li IA IIA IIIA 2, 1 2, 2 2, 3

  43. 11 5 13 7 12 6 B N C IIIA IVA VA 2, 3 2, 4 2, 5

  44. 1 1 4 2 H He 9 4 Be 20 10 7 3 Ne Li 40 18 Ar 24 12 Mg 23 11 Na IA IIA VIIIA 2, 1 2, 2 2, 8 2, 8, 8 2, 8, 1 2, 8, 2

  45. 1 1 1 H 9 4 11 5 Be B 7 3 Li 24 12 Mg 27 13 23 11 Al Na Valence electrons Where most chemical Reactions occur. 2 3 2, 3 2, 1 2, 2 2, 8, 3 2, 8, 1 2, 8, 2

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